Answer:
The final total pressure in the bulb will be 0.567 atm.
Explanation:
The equation of the reaction is:
Ni + 4CO → Ni(CO)₄
The pressure in the bulb will be the sum of the pressures of each gas (remaining CO and Ni(CO)₄ produced).
The pressure of each gas can be calculated using this equation:
For the gas Ni(CO)₄:
P(Ni(CO)₄) = n * R * T / V
where:
P(Ni(CO)₄) = pressure of Ni(CO)₄
n = number of moles of Ni(CO)₄.
R = gas constant = 0.082 l amt / K mol
T = temperature
V = volume
So we have to find how many moles of Ni(CO)₄ were produced and how many moles of CO remained unreacted.
We can calculate the initial number of moles of CO with the data provided in the problem:
P(CO) = n * R * T / V
solving for n:
P(CO) * V / R * T = n
Replacing with the data:
1.20 atm * 1.50 l / 0.082 (l atm / K mol) * 346K = n
n = 0.06mol.
Now we know how many moles of CO were initially present.
To know how many moles of Ni(CO)₄ were produced, we have to find how many Ni reacted with CO.
Initially, we have 0.5869 g of Ni, which is (0.5869 g * 1 mol/58.69 g) 0.01 mol Ni.
From the chemical equation, we know that 1 mol Ni reacts with 4 mol CO, therefore, 0.01 mol Ni will react with 0.04 mol CO producing 0.01 mol Ni(CO)₄ (see the chemical equation above).
At the end of the reaction, we will have 0.01 mol Ni(CO)₄ and (0.06 mol - 0.04 mol) 0.02 mol CO.
Now we can calculate the pressure of each gas after the reaction:
PNi(CO)₄ = n * R * T / V
PNi(CO)₄ = 0.01 mol * 0.082 (l amt / K mol) * 346K / 1.50 l = 0.189 atm
In the same way for CO:
P(CO) = 0.02 mol * 0.082 (l amt / K mol) * 346K / 1.50 l = 0.189 atm = 0.378 atm
The total pressure (Pt) in the bulb, according to Dalton´s law of partial pressures, is the sum of the pressures of each gas in the mixture:
Pt = PNi(CO)₄ + P(CO) = 0.189 atm + 0.378 atm = <u>0.567 atm.</u>
